1. Calculate the pH of a 0.0162 M triethylamine hydrochloride solution. Kb ((C2H5)3N) = 5.6 × 10−4. show work.
2. In a flask, you have 35.00 mL of 0.140 M acetic acid, a weak monoprotic acid with Ka = 1.8 × 10−5. Calculate the pH after the addition of 9.10 mL of 0.140 M NaOH. show work.
1. Calculate the pH of a 0.0162 M triethylamine hydrochloride solution. Kb ((C2H5)3N) = 5.6 ×...
What is the ph of a 0.050 M triethylamine (C2H5) 3N solution? kB for triethylamine is 5.3 x 10^-4 5.32 2.31 1.30 8.68 or 11.69
Salt of a Weak Base and a Strong Acid. pH of Solution. Calculate the pH of a 1.19 M aqueous solution of triethylamine hydrochloride ((C2H5)3NHCI) (For triethylamine, (C2H5)3N, Kb = 4.00x 10-4.) Give two decimal places in your answer.
Given the following information: formic acid HCOOH Ka = 1.8×10-4 triethylamine (C2H5)3N Kb = 5.2×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.167 Maqueous formic acid and triethylamine are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion. -reactant or product favored? -pH is >, <, = to 7?
Determine the pH during the titration of 39.9 mL of 0.349 M triethylamine ((C2H5)3N , Kb = 5.2×10-4) by 0.349 M HBr at the following points. (a) Before the addition of any HBr (b) After the addition of 17.7 mL of HBr (c) At the titration midpoint (d) At the equivalence point (e) After adding 61.0 mL of HBr
Determine the pH during the titration of 39.8 mL of 0.293 M triethylamine ((C2H5)3N, Kb = 5.2×10-4) by 0.293 M HI at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI (b) After the addition of 16.2 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 58.1 mL of HI
1- Determine the pH during the titration of 39.4 mL of 0.374 M triethylamine ((C2H5)3N , Kb = 5.2×10-4) by 0.374 M HClO4 at the following points. (a) Before the addition of any HClO4 (b) After the addition of 16.2 mL of HClO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 55.6 mL of HClO4
1. Calculate the pH of a 0.543 M aqueous solution of codeine (C18H21O3N, Kb = 8.9×10-7). pH = 2. Calculate the pH of a 0.1250 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3). pH = 3. Calculate the pH of a 0.0774 M aqueous solution of the weak base triethylamine ((C2H5)3N, Kb = 5.20×10-4). pH =
A 27.8 mL sample of 0.373 M triethylamine, (C2H5)3N, is titrated with 0.383 M hydrobromic acid. At the equivalence point, the pH is ?
A 25.0 mL sample of 0.291 M triethylamine, (C2H5)3N, is titrated with 0.228 M hydroiodic acid. At the titration midpoint, the pH is ?
A 26.5 mL sample of 0.258 M triethylamine, (C2H5)3N, is titrated with 0.289 M hydroiodic acid. (1) Before the addition of any hydroiodic acid, the pH is (2) After adding 10.5 mL of hydroiodic acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 34.8 mL of hydroiodic acid, the pH is